Year 10 Atomic structure summary

Question 1

What concept did John Dalton introduce?

Answer 1

All matter is composed of small particles called atoms.

Question 2

What model did J.J. Thomson introduce?

Answer 2

The plum pudding model.

Question 3

What analogy did Ernest Rutherford use to describe the atom?

Answer 3

Atoms are like planets orbiting the sun.

Question 4

What particle did James Chadwick discover?

Answer 4

The neutron.

Question 5

What is the relative mass of a proton?

Answer 5

1.

Question 6

What is the relative charge of a proton?

Answer 6

+1.

Question 7

Where is a neutron located?

Answer 7

In the nucleus.

Question 8

What is the relative mass of an electron?

Answer 8

-1.

Question 9

Where is an electron located?

Answer 9

In the shells.

Question 10

What is the atomic number?

Answer 10

The number of protons in the nucleus of an atom.

Question 11

What does the mass number represent?

Answer 11

The sum total of the number of protons and neutrons.

Question 12

How do you find the number of neutrons in an atom?

Answer 12

Mass number - atomic number.

Question 13

What is the electronic configuration of a neon atom?

Answer 13

2.8.

Question 14

What is the maximum number of electrons the first shell can hold?

Answer 14

2.

Question 15

What is the maximum number of electrons the second shell can hold?

Answer 15

8.

Question 16

What is the maximum number of electrons the third shell can hold?

Answer 16

8.

Question 17

What are isotopes?

Answer 17

Elements with the same number of protons but different numbers of neutrons.

Question 18

What is the atomic number of hydrogen (H)?

Answer 18

1.

Question 19

How many neutrons does hydrogen-2 (2H) have?

Answer 19

1.

Question 20

What is the abundance of chlorine-35?

Answer 20

74%.

Question 21

What is the abundance of chlorine-37?

Answer 21

26%.

Question 22

What charge do positive ions have?

Answer 22

Positive charge.

Question 23

What charge do negative ions have?

Answer 23

Negative charge.

Question 24

What do metals tend to do to form ions?

Answer 24

Lose electrons.

Question 25

What do non-metals tend to do to form ions?

Answer 25

Gain electrons.

Question 26

What is the formula for calculating relative atomic mass?

Answer 26

Relative atomic mass = ((% abundance × mass of isotope 1) + (% abundance × mass of isotope 2)) / (total % abundance) ## Footnote This formula is used to find the weighted average of the isotopes of an element based on their natural abundance.

Question 27

Fill in the blank: Relative atomic mass is calculated by taking the weighted average based on _______.

Answer 27

% abundance ## Footnote The percentage abundance refers to how much of each isotope is present in a sample.

Question 28

What does the term 'isotope' refer to in the context of relative atomic mass?

Answer 28

Isotope refers to variants of a chemical element that have the same number of protons but different numbers of neutrons ## Footnote Isotopes have different masses due to the differing number of neutrons.

Question 29

True or False: The total % abundance in the relative atomic mass formula is the sum of the abundances of all isotopes.

Answer 29

True ## Footnote The total % abundance must equal 100% when considering all isotopes of an element.

Question 30

What is the significance of using % abundance in the calculation of relative atomic mass?

Answer 30

It ensures that the mass reflects the natural occurrence of each isotope ## Footnote This is important for accurate representation of the element's atomic mass in nature.

Question 31

List two factors that contribute to the calculation of relative atomic mass.

Answer 31

* % abundance of isotopes * Mass of isotopes ## Footnote Both factors are essential for determining the weighted average atomic mass.